Calculate the pH of a solution containing a salt AcNa derived from a strong base (NaOH) and a weak acid (AcH), like CH3COONa, KF, NaNO2 and so on. In this case two processes have to be considered: 1. Dissociation of the salt, within the assumption that the salt is a strong electrolyte: AcNa → Ac- + Na+, for instance: CH3COONa → CH3COO- + Na+ 2. the hydrolysis of the water Ac- + H2O ⇌ AcH + OH-, for example: CH3COO- + H2O ⇌ CH3COOH + OH- knowing that the initial concentration of the salt is 1.95 M and the acid dissociation constant, Ka , is 1.21e-7.

Calculate the pH of a solution containing a salt AcNa derived from a strong base (NaOH) and a weak acid (AcH), like CH3COONa, KF, NaNO2 and so on. In this case two processes have to be considered: 1. Dissociation of the salt, within the assumption that the salt is a strong electrolyte: AcNa → Ac- + Na+, for instance: CH3COONa → CH3COO- + Na+ 2. the hydrolysis of the water Ac- + H2O ⇌ AcH + OH-, for example: CH3COO- + H2O ⇌ CH3COOH + OH- knowing that the initial concentration of the salt is 1.95 M and the acid dissociation constant, Ka , is 1.21e-7.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 107AP

See similar textbooks

Similar questions

Calculate the pH of a solution containing a salt AcNa derived from a strong base (NaOH) and a weak acid (AcH), like CH3COONa, KF, NaNO2 and so on. In this case two processes have to be considered: 1. Dissociation of the salt, within the assumption that the salt is a strong electrolyte: AcNa → Ac- + Na+, for instance: CH3COONa → CH3COO- + Na+ 2. the hydrolysis of the water Ac- + H2O ⇌ AcH + OH-, for example: CH3COO- + H2O ⇌ CH3COOH + OH- knowing that the initial concentration of the salt is 1.75 M and the acid dissociation constant, Ka , is 2.07e-7. What is the PH?
The pH factor is a measure of the acidity and alkalinity of water. A reading of 7.0 is neutral; values in excess of 7.0 indicate alkalinity; those below 7.0 imply acidity. In one study, it is mentioned that the best chance of catching bass occurs when the pH of the water is in the range 7.5 to 7.9. Suppose your suspect that acid rain is lowering the pH of your favourite fishing spot and you wish to determine whether the pH is less than 7.5. You obtained 10 samples and got the following data: 7.3, 7.4, 7.2, 7.0, 7.5,7.4,7.3,7.3,7.2 and 7.1. Use 0.05 alpha. a. State the alternative and null hypothesis. b. Is the pH of the water samples less than 7.5?
How to answer for Ka/ Kb and calculated pH of a solution? I think solution 1,2 only has one Ka/Kb value then the other Sol. 3,4. Then with calculated pH, pH = -log[H+] (acid) and pH = 14 + log[OH-] (base) is utilized. Though I do not know how getting the Ka/Kb will be used to get pH Ex. Solution 1: 30.0 mL 0.10 M CH3COOHSolution 2: 15.0 mL 0.20 M CH3COOH – 15.0 mL 0.20 M NaCH3COOSolution 3: 30.0 mL 0.10 M NH3Solution 4: 15.0 mL 0.20 M NH3 – 15.0 mL 0.20 M NH4Cl Sol 1,2 used methyl orange as indicatorSol 3,4 used phenolphthalein as indicator Solution w/ measured pH Ka/Kb Calculated pH 1 a 1.0 M HCl (2.01pH) b 1.0 M NaOH (3.98pH) c Control (2.91pH) 2 a 1.0 M HCl (4.73) b 1.0 M NaOH (4.82) c Control (4.76) 3. a 1.0 M HCl (10.09) b 1.0 M NaOH (11.98) c Control (11.11) 4. a 1.0 M HCl (9.13) b 1.0 M NaOH (9.38) c Control (9.30)
Calculate the pH of two HCl solution based on their concentrations of 0.001 and0.0001 M. Then calculate the pH of a solution when you add each of these to a closed carbonicacid system with mcarb-t = mH2CO3 + mHCO3- + mCO32- = 0.01 m and pH = 6. At that pH, mH2CO3 =10-2.16; mHCO3- =10-2.51; mCO32- is negligible.
The pH and electrical conductivity of four different mixtures were measured: Mixtures conductivity (mA) pH a. 0.1 mol L-1 HCI 260 1 B. 0.1 mol L-1 CH3COOH 5 3 c. Mixture made by mixing equal volumes of 0.2 mol L-1 HCI and 0.2 mol L-1 NaCl 340 1 D. Mixture made by mixing equal volumes of 0.2 mol L-1 HCI and 0.2 mol L-1 NaCH3COO 80 3 a. Explain why the conductivity of mixture a is higher than that of mixure b, yet the pH of a is lower than the pH of B. Include relevant equations in your answer b. Explain why the pH of mixture C is the same as the pH of mixture A c. Why is the conductivity of mixture C larger than the conductivity of mixture A d. Why is the pH of mixture D the same as the pH of mixture B Determine the final pH for the following two solutions a. solution a after mixing 500 ml 0.2M HCl and 300 ml 0.6M Hcl b. solution b after mixing 400ml 0.3M HCl and 200ml 0.8M NaOH
In Experiment 4, we used titration to determine the total acid content of samples, which we reported in terms of molarity. Reporting acidity through pH measurements is quite different, in that we can only measure the amount of the acid in its ionized form. You were tasked to investigate a clear aqueous solution of an unknown monoprotic acid. You decided to use two Chem 16.1 methods to gather data.Method 1 – TITRATION: A 10. mL aliquot of the sample was diluted with 25 mL distilled water. Two drops of phenolphthalein were added and then it was titrated 3.54 mL of 0.048 M standardized NaOH to the endpoint.Method 2 – pH STRIP: You took 1 mL of the sample and used a pH strip to estimate the pH, which turned out to be around 3.3. Another 1 mL of the sample was diluted with 9 mL of water. The pH was taken again and is now around 3.8 a) Calculate the molarity of the acid using the titration data.b) If we assume that the titrated unknown is a strong acid, predict the pH of the sample.c) Using…
In Experiment 4, we used titration to determine the total acid content of samples, which we reported in terms of molarity. Reporting acidity through pH measurements is quite different, in that we can only measure the amount of the acid in its ionized form. You were tasked to investigate a clear aqueous solution of an unknown monoprotic acid. You decided to use two Chem 16.1 methods to gather data.Method 1 – TITRATION: A 10. mL aliquot of the sample was diluted with 25 mL distilled water. Two drops of phenolphthalein were added and then it was titrated 3.54 mL of 0.048 M standardized NaOH to the endpoint.Method 2 – pH STRIP: You took 1 mL of the sample and used a pH strip to estimate the pH, which turned out to be around 3.3. Another 1 mL of the sample was diluted with 9 mL of water. The pH was taken again and is now around 3.8 d) Based on your answer in a) and c), do you think the unknown is really a strong acid or is it a weak acid instead? Defend your answer in one sentence.e)…
The pH and electrical conductivity of four different mixtures were measured:Mixtures Conductivity(mA)pHA 0.1 mol L–1 HCl 260 1B 0.1 mol L–1 CH3COOH 5 3C Mixture made by mixing equal volumes of0.2 mol L–1 HCl and 0.2 mol L–1 NaCl340 1D Mixture made by mixing equal volumes of0.2 mol L–1 HCl and 0.2 mol L–1 NaCH3COO80 3 Explain why the conductivity of mixture A is higher than that of mixture B, yet the pH of A is lower than the pH of B. Include relevant equations in your answer. Explain why the pH mixture of C is the same as the pH mixture of A. Why is the conductivity of mixture C larger than the conductivity of mixture A? Why is the pH of mixture D the same as the pH of mixture B?
the pH and electrical conductivity of four different mixtures were measured mixtures conductivity (mA) pH a. 0.1 mol L-1 HCl 260 1 b. 0.1 mol L-1 CH3COOH 5 3 c. mixture made by mixing equal volumes of 0.2 mol L-1 HCl and 0.2 mol L-1 NaCl 340 1 d. mixture made by mixing equal volumes of 0.2 mol L-1 HCl and 0.2 mol L-1 NaCH3COO 80 3 Determine the final pH for the following two solutions a) solution A after mixing 500ml 0.2M HCl and 300ml 0.6M HCl b) solution B after mixing 400 ml 0.3M HCl and 200 ml 0.8M HCl
the pH and electrical conductivity of four different mixtures were measured mixtures conductivity (mA) pH a. 0.1 mol L-1 HCl 260 1 b. 0.1 mol L-1 CH3COOH 5 3 c. mixture made by mixing equal volumes of 0.2 mol L-1 HCl and 0.2 mol L-1 NaCl 340 1 d. mixture made by mixing equal volumes of 0.2 mol L-1 HCl and 0.2 mol L-1 NaCH3COO 80 3 C. Why is the conductivity of mixture C larger than the conductivity of mixture a? D. Why is the pH of mixture D the same as the pH for mixture B?
Determine the pH of a solution that is prepared by dissolving 5.2 g of Ba(OH)2 in 2.8 L water at 25°C. Assume that the volume of the solvent does not change upon addition of the solute. Atomic Weights: Ba = 137.3 g/mol; O = 16.00 g/mol; H = 1.008 g/mol. Express your answer in two decimal places only. Do not put the units.
Consider a 0.10 M solution of a weak polyprotic acid (H2A) with the possible values of Ka1 and Ka2 given below. Calculate the contributions to [H3O+] from each ionization step. a) Ka1=1.0×10−4;Ka2=5.0×10−5 Express your answers using two significant figures separated by commas. b) Ka1=1.0×10−4;Ka2=1.0×10−5 Express your answers using two significant figures separated by commas. c) Ka1=1.0×10−4;Ka2=1.0×10−6 Express your answers using two significant figures separated by commas.